process has delta H = -87.4 kj. a) calculate delta S surroundings of the process at...
process has delta H = -87.4 kj.
a) calculate delta S surroundings of the process at 204 K
b) if delta S system for the same process is 18.7 J/K, how much energy is available to do work at 298 K? assume delta H process is constant through temperature range
c) could that much energy (part b) actually be utilized for work? why or why not
Homework Answers
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process has delta H = -87.4 kj.
a) calculate delta S surroundings of the process at...
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate...
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
If the delta H of a certain reaction is -623 kJ/mole and the delta S is...
If the delta H of a certain reaction is -623 kJ/mole and the delta S is -114 J/mole K What is the temperature range for which this reaction is spontaneous
A) For the reaction 4HCl(g) + O2(g)---->2H2O(g) + 2Cl2(g) Delta H° = -114.4 kJ and Delta...
A) For the reaction 4HCl(g) + O2(g)---->2H2O(g) + 2Cl2(g) Delta H° = -114.4 kJ and Delta S° = -128.9 J/K The equilibrium constant for this reaction at 306.0 K is _______? Assume that Delta H° and DeltaS° are independent of temperature. B) For the reaction N2(g) + 3H2(g)---->2NH3(g) Delta H° = -92.2 kJ and Delta S° = -198.7 J/K The equilibrium constant for this reaction at 333.0 K is ___? Assume that Delta H° and Delta S° are independent of...
A certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50...
A certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50 J/K. Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to in the disorder of the system. Calculate Delta G degree for this reaction at 298 K. If this value is less than 1 kJ/mol then enter 0 in...
A 0.0403 M solution of a particular monoprotic weak acid. HA, has a pH of 3,...
A 0.0403 M solution of a particular monoprotic weak acid. HA, has a pH of 3, 40 a 298 K. What is Delta G^Compositefunction for the following equilibrium? HA (aq) + H_2O(l) rightarrow leftarrow H_2O(aq) = A(aq) A) 7.95 kJ B) 30.8 kJ C) 11.4 kJ D) 19.4 kJ For a reversible phase change at constant temperature and pressure. A) Delta U = 0. B) Delta H = 0. C) w = 0 D) q = 0 E) Delta G...
If, for a particular process, delta H = -214 kJ/mol and delta S = 450 J/mole...
If, for a particular process, delta H = -214 kJ/mol
and delta S = 450 J/mole K, the process will be. Please show work
too, I am trying hard to understand!
< > Options Due Monday, Nov 25, 11:59pm EST © Explain how spontaneity is affected by temperature Question If, for a particular process, AH = -214 and AS - 450k the process will be: Select the correct answer below: O spontaneous at any temperature O nonspontaneous at any temperature...
a reaction has delta H = 100.0 kJ/mol and delta S = 250.0 J/mol K. Is...
a reaction has delta H = 100.0 kJ/mol and delta S = 250.0 J/mol K. Is the reaction spontaneous at room temperature? If no, at what temperature (in K and C) does this reaction become spontaneous?
A reaction has a delta H^0_Txn= -167.5 kJ/mol and delta S^0_Txn = 57.3 J/mo\ K. Calculate...
A reaction has a delta H^0_Txn= -167.5 kJ/mol and delta S^0_Txn = 57.3 J/mo\ K. Calculate the equilibrium constant for the reaction. What is the difference between thermodynamic equilibrium constant and the apparent equilibrium constant?
8.) From the values of delta H and delta S, calculate delta G then predict whether...
8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol
For a particular chemical reaction Delta H = 6.5 kJ and Delta S = -33 J/K....
For a particular chemical reaction Delta H = 6.5 kJ and Delta S = -33 J/K. Under what temperature condition is the reaction spontaneous? When T> 197 K. When T< 197 K. The reaction is not spontaneous at any temperature. When T < -197 K. The reaction is spontaneous at all temperatures.
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
A certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50 J/K. Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to in the disorder of the system. Calculate Delta G degree for this reaction at 298 K. If this value is less than 1 kJ/mol then enter 0 in...
A 0.0403 M solution of a particular monoprotic weak acid. HA, has a pH of 3, 40 a 298 K. What is Delta G^Compositefunction for the following equilibrium? HA (aq) + H_2O(l) rightarrow leftarrow H_2O(aq) = A(aq) A) 7.95 kJ B) 30.8 kJ C) 11.4 kJ D) 19.4 kJ For a reversible phase change at constant temperature and pressure. A) Delta U = 0. B) Delta H = 0. C) w = 0 D) q = 0 E) Delta G...
If, for a particular process, delta H = -214 kJ/mol
and delta S = 450 J/mole K, the process will be. Please show work
too, I am trying hard to understand!
< > Options Due Monday, Nov 25, 11:59pm EST © Explain how spontaneity is affected by temperature Question If, for a particular process, AH = -214 and AS - 450k the process will be: Select the correct answer below: O spontaneous at any temperature O nonspontaneous at any temperature...
A reaction has a delta H^0_Txn= -167.5 kJ/mol and delta S^0_Txn = 57.3 J/mo\ K. Calculate the equilibrium constant for the reaction. What is the difference between thermodynamic equilibrium constant and the apparent equilibrium constant?
8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol
For a particular chemical reaction Delta H = 6.5 kJ and Delta S = -33 J/K. Under what temperature condition is the reaction spontaneous? When T> 197 K. When T< 197 K. The reaction is not spontaneous at any temperature. When T < -197 K. The reaction is spontaneous at all temperatures.
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